What is the concentration of iron(II) sulfide in water at 25 °C? Ksp for iron(II) sulfide...
What is the concentration of iron(II) ions in a saturated solution of iron(II) sulfide? Ksp(FeS) = (3.765x10^-19) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: Question 68 options: x10 Answer units
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80× 10−14 Part C What will the concentration of Cd2+ at the moment before Fe2+ begins to precipitate? Express your answer with the appropriate units.
The equilibrium concentration of iron(II) ion in a saturated iron(II) sulfide solution is M .
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80×10−14 A solution of Na2CO3 is added dropwise to a solution that contains 1.21×10−2MFe2+ and 1.45×10−2M Cd2+. What concentration of CO32− is need to initiate precipitation? Neglect any volume changes during the addition. Express the molar concentration numerically.
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80×10−14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.20×10−2 M Fe2+ and 1.60×10−2 M Cd2+. What will the concentration of Cd2+ at the moment before Fe2+ begins to precipitate?
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Ksp FeCO3 2.10×10−11 CdCO3 1.80× 10−14 A solution of Na2CO3 is added dropwise to a solution that contains 1.00×10−2 M Fe2+ and 1.49×10−2 M Cd2+. What concentration of CO32− is need to initiate precipitation? Neglect any volume changes during the addition.
Please help ASAP! 1. Solid iron(II) carbonate and solid iron(II) sulfide are in equilibrium with a solution containing 1.21×10-2 M sodium carbonate. Calculate the concentration of sulfide ion present in this solution. [sulfide] = ________ M 2. Solid manganese(II) sulfide and solid copper(II) sulfide are in equilibrium with a solution containing 1.31×10-2 M manganese(II) nitrate. Calculate the concentration of copper(II) ion present in this solution. [copper(II)] = _______ M 3. Consider these compounds: A. Al(OH)3 B. Cr(OH)3 C. Ag2CrO4 D....
The equilibrium concentration of iron(III) ion in a saturated iron(III) sulfide solution is ___ M. (the Ksp is given as 1.4 × 10-88)
ksp
= 4 x 10-20
access important The molar solubility of nickel(II) sulfide in a water solution is Submit Answer Retry Entire Group 4 more group attempts remaining
QUESTION 3 At 25 °C the solubility of mercury(II) sulfide is 1.26 x 10-26 mol/L. Calculate the value of Ksp at this temperature. Give your answer in scientific notation to 2 SIGNIFICANT FIGURES (even though this is strictly incorrect).